Sunday
April 20, 2014

Homework Help: Chemistry - molecular polarity

Posted by Constantine on Thursday, April 18, 2013 at 3:45pm.

Hi Dr. Bob. Could you please take a look at the question below and my work? I'm not sure how to get the correct answer for this question. I would greatly appreciate your help!

How many of the following molecules are polar?

BrCl3
CS2
SiF4
SO3

A) 1
B) 2
C) 3
D) 4
E) 0


The correct answer for this question is A) which is 1. However I could not find a polar molecule among the ones given.

BrCl3: the molecule has a T-shaped molecular geometry which could make it polar, but the Br-Cl electronegativity difference is 0.2 which makes it a covalent bond.

CS2: the molecule has a linear geometry and the electronegativity difference between C and S is 0, so this one is not polar either.

SiF4: the molecule has a tetrahedral molecular geometry so even though the S-iF electronegativity large and the bond is polar covalent, the bonds cancel each other out.

SO3: the molecule has a trigonal planar molecular geometry so the S-O bonds cancel each other out.

Could you please let me know which molecule is polar and why?

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